Student ID: 38982299 15. Good practice. Sulfur has amongst the most diverse chemistry of all of the atoms of the periodic table. For example, it forms a large number of different compounds in the presence of oxygen, including SO2, SO3, SO32- and SO42. In each of these molecules, the S-O bond distances are different, as can be seen in the table at right. Provide a rationale for the reported bond distances for each of these species. Molecule rso (pm) Sulfur dioxide SO2 144 Sulfur trioxide SO3 142 Sulphite [SO3]²- 152 Sulphate [SO4]²- 149

Student ID: 38982299 15. Good practice. Sulfur has amongst the most diverse chemistry of all of the atoms of the periodic table. For example, it forms a large number of different compounds in the presence of oxygen, including SO2, SO3, SO32- and SO42. In each of these molecules, the S-O bond distances are different, as can be seen in the table at right. Provide a rationale for the reported bond distances for each of these species. Molecule rso (pm) Sulfur dioxide SO2 144 Sulfur trioxide SO3 142 Sulphite [SO3]²- 152 Sulphate [SO4]²- 149

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter3: Atomic Shells And Classical Models Of Chemical Bonding

Section: Chapter Questions

Problem 38P: The percent ionic character of the bonds in several interhalogen Molecules (as estimated from their...

See similar textbooks

Similar questions

Base on the chemical equation of the Haber process ½ N2(g) + 3/2 H2(g) = NH3(g), estimate DfH, for ammonia using bond dissociation energies. [DbondH,/ kJ mol–1: H–H = 436; NºN = 945; N–H = 391] Select one: a. –46.5 kJ mol–1 b. 735.5 kJ mol–1 c. –93.0 kJ mol–1 d. 93.0 kJ mol
Each of the following properties shows a regular trend inGroup 1A(1). Predict whether each increases or decreases downthe group: (a) density; (b) ionic size; (c) E−E bond energy; (d) IE₁; (e) magnitude of ΔH(hydr) of E⁺ion.
Explain why :(i) No chemical compound of helium is known.(ii) Bond dissociation energy of fluorine is less than that of chlorine.(iii) Two S–O bonds in SO2are identical.
The element xenon (Xe) is by no means chemically inert;it forms a number of chemical compounds with electronegative elements such as fluorine and oxygen. The reaction of xenon with varying amounts of fluorine producesXeF2 and XeF4. Subsequent reaction of one or the otherof these compounds with water produces (depending onconditions) XeO3, XeO4, and H4XeO6, as well as mixedcompounds such as XeOF4. Predict the structures ofthese six xenon compounds, using the VSEPR theory.
Average Bond Dissociation Energies at 298 K Bond Energy, kJ mol1 H-H 432 O=0 495 H-O 467 The tables above contain information for determining thermodynamic properties of the reaction below. 2H,(g) + 02(8) - 2H,O(g) (a) Calculate the AH° for the reaction above, using the table of average bond dissociation energy. (b) Use the table below to calculate the entropy for the formation of water. 2H, + 02 - 2H,O Substance S°(J/mol· K) H2 131.0 H20 69.91 O2 205.0 (c) Calculate the value of AG°298K for the synthesis of water.
Chlorine dioxide gas (ClO2) is used as a commercial bleachingagent. It bleaches materials by oxidizing them. In thecourse of these reactions, the ClO2 is itself reduced. (a)What is the Lewis structure for ClO2? (b) Why do you thinkthat ClO2 is reduced so readily? (c) When a ClO2 moleculegains an electron, the chlorite ion, ClO2-, forms. Draw theLewis structure for ClO2-. (d) Predict the O—Cl—O bondangle in the ClO2- ion. (e) One method of preparing ClO2is by the reaction of chlorine and sodium chlorite:Cl2(g) + 2 NaClO2(s)------>2 ClO2(g) + 2 NaCl(s)If you allow 15.0 g of NaClO2 to react with 2.00 L of chlorinegas at a pressure of 1.50 atm at 21 °C, how many gramsof ClO2 can be prepared?
The percent ionic character of the bonds in several interhalogen Molecules (as estimated from their measured dipole moments and bond lengths) are ClF (11%), BrF(15%), BrCl (5.6%), ICl(5.8%), and IBr (10%). Estimate the percent ionic characters for each of these molecules, using the equation in Problem 37, and compare them with the given values.
Thionyl chloride (SOCl₂) is a sulfur oxohalide used indus-trially to dehydrate metal halide hydrates. (a) Write a balancedequation for its reaction with magnesium chloride hexahydrate,in which SO₂ and HCl form along with the metal halide. (b) Drawa Lewis structure of SOCl₂ with minimal formal charges.
AutoSave Module 4; Lewis Structures of Covalent Compounds - Saved to this PC P Searc Off File Home Insert Draw Design Layout References Mailings Review View Help Grammarly Times New Roma v 12 A A Aa v AaBbCcI AaBbCcI Aa Paste в IU ab х, х* А A I Normal I No Spac.. Hea Clipboard Font Paragraph 4..| 5 9... |·· 10. . |. 11. ..| 12. . | 13... 14. 15. * The speaker uses the term "lone electron pair" instead of non-bonding electron pair. It is the same thing. **Number VESPR Groups is equal to the number of atoms bonded to the central atom plus the mumber oaf ncn-bonding pairs. Draw the Lenis structure Name the shape. ihoning the correct :kape. LUse element symbols, dots for ncn- bonding electron pairs and dashes for banded electrons. BeCl, со. HCN BF, CH.O so, CH, NH, Number of VESPR
In the sulfate (SO42-) anion, all the S-O bond lengths are the same. Draw suitable resonance structures to explain this observation. Sulfite (SO32-) anions also have S-O bonds of equal lengths but these are different to sulfate lengths. Identify the system with the shorter bond length and explain your reasoning.
In the series of group 5A hydrides, of general formulaMH3, the measured bond distances are P¬H, 1.419 Å;As¬H, 1.519 Å; Sb¬H, 1.707 Å. (a) Compare these valueswith those estimated by use of the atomic radii inFigure 7.7. (b) Explain the steady increase in M¬H bonddistance in this series in terms of the electron configurationsof the M atoms.
Assuming acid strength relates directly to number of O atoms bonded to the central atom, rank H₂N₂O₂[or (HON)₂];HNO₃(or HONO₂); and HNO₂(or HONO) in order of decreasing acid strength